Which of the following exhibits the highest boiling point?

Ne, Ar, Kr, or Xe
My answer: Xe

Which of the following exhibits the highest boiling point?
F2, Cl2, Br2, or I2
My answer: HI

Which of the following exhibits the highest boiling point?
NaCl, SO2, or N2
My answer: SO2

These are my answers because these ones have the highest molecular weight. Are they correct? If not, how do I figure them out?

Your answers are not correct. To determine which substance has the highest boiling point, you need to consider the intermolecular forces of attraction between the molecules. The stronger the intermolecular forces, the higher the boiling point. Molecular weight alone is not enough to determine boiling points.

Let's go through each question and find the correct answers:

1. Which of the following exhibits the highest boiling point? Ne, Ar, Kr, or Xe

The noble gases (Ne, Ar, Kr, Xe) are all monatomic gases with weak van der Waals forces. As we move down the group, the atomic size increases, leading to stronger London dispersion forces. Therefore, Xe would have the highest boiling point among the given options.

2. Which of the following exhibits the highest boiling point? F2, Cl2, Br2, or I2

The halogens (F2, Cl2, Br2, I2) are diatomic molecules bonded by covalent bonds. As we move down the group, the size of the atoms increases, leading to a larger electron cloud and stronger London dispersion forces. Therefore, I2 would have the highest boiling point among the given options.

3. Which of the following exhibits the highest boiling point? NaCl, SO2, or N2

NaCl is an ionic compound consisting of a lattice of positive sodium ions and negative chloride ions. Ionic compounds have strong electrostatic forces of attraction between ions, resulting in high boiling points.

SO2 is a covalent compound with polar covalent bonds. It has dipole-dipole interactions but weaker than ionic bonds, so its boiling point will be lower than NaCl.

N2 is a diatomic molecule with nonpolar covalent bonds, and it only experiences weak London dispersion forces. Therefore, N2 would have the lowest boiling point among the given options.

In summary, when comparing the boiling points, it is essential to consider the nature of the intermolecular forces between the molecules or ions.